Some measurements of the initial rate of a certain reaction are given in the table below.H2 12 initial rate of reaction1.89 M | 0.790м9.00 x 10°M/s2.27 x 10°M/s1.78 x 10° M/s1.89 M | 0.199м|0.373 М 0.790мUse this information to write a rate law for this reaction, and calculate the value of the rate constant k.Round your value for the rate constant to 3 significant digits. Also be sure your answer has the correct unit symbol.rate = k ||k =

Given : Table showing concentration of reactants and rate To find : Rate law and rate constant…

Answered: Some measurements of the initial rate…

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter12: Chemical Kinetics

Section: Chapter Questions

Problem 5ALQ: Consider the following statements: In general, the rate of a chemical reaction increases a bit at...

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Consider the following statements: In general, the rate of a chemical reaction increases a bit at first because it takes a while for the reaction to get warmed up. After that, however, the rate of the reaction decreases because its rate is dependent on the concentrations of the reactants, and these are decreasing. Indicate everything that is correct in these statements, and indicate everything that is incorrect. Correct the incorrect statements and explain.
Consider a hypothetical reaction between A and B: A + B products Use the following initial rate data to calculate the rate constant for this reaction. [A] (mol/L) [B] (mol/L) Initial Rate (mol/L s) 0.20 1.0 3.0 0.50 1.0 11.8 2.0 2.0 189.5
In Exercise 11.39, if the initial concentration of N2Oj is 0.100 .\1. how long will it take for the concentration to drop to 0.0100 times its original value? The decomposition of N2O5 in solution in carbon tetrachloride is a first-order reaction: 2N2O5—»4NO2 + O2 The rate constant at a given temperature is found to be 5.25 X 10-4 s-’. If the initial concentration of N2O5 is 0.200 M, what is its concentration after exactly 10 minutes have passed?
Experimental data are listed here for the reaction B: Time (s) IB] (mol/L) 0.00 0.000 10.0 0.326 20.0 0.572 30.0 0.750 40.0 0.890 Prepare a graph from these data, connect the points with a smooth line, and calculate the rate of change of [B] for each 10-s interval from 0.0 to 40.0 s. Does the rate of change decrease from one time interval to the next? Suggest a reason for this result. How is the rate of change of [AJ related to the rate of change of [B] in each time interval? Calculate the rate of change of [AJ for the time interval from 10.0 to 20.0 s. What is the instantaneous rate, A[B]/Ar, when [BI = 0.750 mol/L?
You are running the reaction 2A+BC+3D. Your lab partner has conducted the first two experiments to determine the rate law for the reaction by the method of initial rates. Experiment Number Concentration of A (M) Concentration of B(M) 1 0.0250 0.0330 2 0.0500 0.0330 3 Presuming that you can measure the initial rate of each experiment, which of the following concentrations for Experiment 3 would help you determine the rate law easily? a [A] = 0.0330 M, [B] = 0.0330 M b [A] = 0.0125 M, [B] = 0.0500 M c [A] = 0.0250 M, [B] = 0.0400 M d [A] = 0.0250 M, [B] = 0.0330 M e [A] = 0.0500 M, [B] = 0.0330 M
Based on the kinetic theory of matter, what would the action of a catalyst do to a reaction that is the reverse of some reaction that we say is catalyzed?
Consider the following hypothetical data collected in two studies of the reaction 2A+2BC+2D Time(s) Experiment 1 [A] (mol/L) Experiment 2 [A] (mol/L) 0 1.0 102 1.0 102 10. 8.4 103 5.0 103 20. 7.1 103 2.5 103 30. ? 1.3 103 40. 5.0 103 6.3 104 In Experiment 1, [B]0 = 10.0 M. In Experiment 2, [B]0 = 20.0 M. Rate=[A]t a. Use the concentration versus time data to determine the rate law for the reaction. b. Solve for the value of the rate constant (k) for the reaction. Include units. c. Calculate the concentration of A in Experiment 1 at t =30.s
The following statements relate to the reaction for the formation of HI: H2(g) + I2(g) -* 2 HI(g) Rate = it[HJ [I2J Determine which of the following statements are true. If a statement is false, indicate why it is incorrect. The reaction must occur in a single step. This is a second-order reaction overall. Raising the temperature will cause the value of k to decrease. Raising the temperature lowers the activation energy' for this reaction. If the concentrations of both reactants are doubled, the rate will double. Adding a catalyst in the reaction will cause the initial rate to increase.
At 40C, H2O2 (aq) will decompose according to the following reaction: 2H2O2(aq)2H2O(l)+O2(g) The following data were collected for the concentration of H2O2 at various times. Times(s) [H2O2](mol/L) 0 1.000 2.16 104 0.500 4.32 104 0.250 a. Calculate the average rate of decomposition of H2O2 between 0 and 2.16 104 s. Use this rate to calculate the average rate of production of O2(g) over the same time period. b. What are these rates for the time period 2.16 104 s to 4.32 104 s?
Experiments show that the reaction of nitrogen dioxide with fluorine, 2 NO2(g) + F2(g) —* 2 FNO2(g) has the rate law Rate = *[NO2][FJ The reaction is thought to occur in two steps. Step 1: NO2(g) + F,(g) —* FNO,(g) + F(g) Step 2: NO2(g) + F(g) — FNO2(g) Show that the sum of this sequence of reactions gives the balanced equation for the overall reaction. Which step is rate determining?
For each of the rate laws below, what is the order of the reaction with respect to the hypothetical substances X, Y, and Z? What is the overall order? (a) Rate = k [X][Y][Zl, (b) Rate = k [X]-[Y]1/2[Z], (c) Rate = k [X]L5[Y]-1, (d) Rate = k [X]/[Y]2
Experimental data are listed here for the reaction A 2 B. (a) Prepare a graph from these data; connect the points with a smooth line; and calculate the rate of change of [B] for each 10-second interval from 0.0 to 40.0 seconds. Does the rate of change decrease from one time interval to the next? Suggest a reason for this result. (b) How is the rate of change of [A] related to the rate of change of [B] in each time interval? Calculate the rate of change of [A] for the time interval from 10.0 to 20.0 seconds.

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